Stoichiometry of Solution Reactions
I. VIDEO ON SOLUTION STOICHIOMETRY
II. NOTES ON SOLUTION STOICHIOMETRY
III. EXERCISES ON SOLUTION STOICHIOMETRY
1. Calculate the mass of solid NaCl that must be added to 1.50 L of a 0.100 M AgNO3 solution to precipitate
all of the Ag+ ions in the form of AgCl. Calculate the mass of AgCl formed.
2. Calculate the mass of solid sodium sulfate that must be added to 250.0 mL of a 0.200 M solution of barium
nitrate to precipitate all of the barium ions in the form of barium sulfate. Also calculate the mass of
barium sulfate formed.
3. Calculate the mass of NaI that must be added to 425.0 mL of a 0.100 M Pb(NO3)2 solution to precipitate
all of the Pb2+ ions as PbI2. Also calculate the mass of PbI2 formed.
4. When Ba(NO3)2 and K2CrO4 react in aqueous solution, the yellow solid BaCrO4 is formed. Calculate the
mass of BaCrO4 that forms when 3.50 x 10-3 mol of solid Ba(NO3)2 is dissolved in 265 mL of 0.0100 M
K2CrO4 solution.
5. Calculate the mass of the white solid CaCO3 that forms when 25.0 mL of a 0.100 M Ca(NO3)2
solution is mixed with 20.0 mL of a 0.150 M Na2CO3 solution.
6. When aqueous solutions of Na2SO4 and Pb(NO3)2 are mixed, PbSO4, precipitates. Calculate the mass
of PbSO4 formed when 1.25 L of 0.0500 M Pb(NO3)2 and 2.00 L of 0.0250 M Na2SO4 are mixed.
7. Calculate the mass of the blood-red solid Ag2CrO4 that forms when 50.0 mL of a 0.250 M AgNO3
solution is mixed with 30.0 mL of a 0.250M K2CrO4 solution.
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